Textbook Question
What are the basic assumptions of the kinetic–molecular theory?
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Ch.10 - Gases: Their Properties & Behavior
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Chapter 10, Problem 91b
Gaseous compound Q contains only xenon and oxygen. When 0.100 g of Q is placed in a 50.0-mL steel vessel at 0 °C the pressure is 0.229 atm. (b) When the vessel and its contents are warmed to 100 °C, Q decomposes into its constituent elements. What is the total pressure, and what are the partial pressures of xenon and oxygen in the container?
Verified step by step guidance1
Determine the initial number of moles of compound Q using the ideal gas law equation: PV = nRT. Here, P is the initial pressure, V is the volume of the container, R is the ideal gas constant (0.0821 L atm K^{-1} mol^{-1}), and T is the initial temperature in Kelvin.
Convert the initial temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature.
Calculate the final temperature in Kelvin by converting 100 °C to Kelvin.
Assume complete decomposition of compound Q into xenon and oxygen. Since the number of moles of gas increases due to decomposition, use stoichiometry based on the chemical formula of Q to determine the ratio in which xenon and oxygen are formed.
Calculate the total pressure at the new temperature using the ideal gas law, considering the total number of moles of xenon and oxygen. Then, use the mole fraction of each gas to find their respective partial pressures.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Ideal Gas Law
The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is essential for calculating the behavior of gases under varying conditions, such as changes in temperature and pressure, which is crucial for solving the problem involving the gaseous compound Q.
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Ideal Gas Law Formula
Decomposition Reactions
Decomposition reactions involve the breakdown of a compound into its constituent elements or simpler compounds. In this scenario, understanding how compound Q decomposes into xenon and oxygen at elevated temperatures is vital for determining the resulting pressures of each gas in the vessel after the reaction occurs.
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Dalton's Law of Partial Pressures
Dalton's Law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of each individual gas. This principle is key to calculating the total pressure and the partial pressures of xenon and oxygen after the decomposition of compound Q in the steel vessel.
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Related Practice
Textbook Question
Gaseous compound Q contains only xenon and oxygen. When 0.100 g of Q is placed in a 50.0-mL steel vessel at 0 °C the pressure is 0.229 atm. (a) What is the molar mass of Q, and what is a likely formula?
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Textbook Question
The average temperature at an altitude of 20 km is 220 K. What is the average speed in m/s of an N2 molecule at this altitude?
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Textbook Question
What is the difference between heat and temperature?
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Textbook Question
Natural gas is a mixture of hydrocarbons, primarily methane (CH4) and ethane (C2H6). A typical mixture might have Xmethane = 0.915 and Xethane = 0.085. Let's assume that we have a 15.50 g sample of natural gas in a volume of 15.00 L at a temperature of 20.00 °C. (c) What is the partial pressure of each component in the sample in atmospheres?
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Textbook Question
Natural gas is a mixture of hydrocarbons, primarily methane (CH4) and ethane (C2H6). A typical mixture might have Xmethane = 0.915 and Xethane = 0.085. Let's assume that we have a 15.50 g sample of natural gas in a volume of 15.00 L at a temperature of 20.00 °C. (b) What is the pressure of the sample in atmospheres?
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